Ammonia is synthesized from nitrogen and hydrogen via the reaction:
N2(g) + 3 H2(g) → 2 NH3(g)
ΔG° at 298 K for this reaction is −33.3 kJ/mol. What is the value of ΔG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 in kJ/mol?
I used the formula DeltaG = ΔG° -RTln(K
K=(.65)2/(1.9x1.63) = .0543
-((8.314)(298)(ln.0543))/1000 = 7.218 kJ
Delta G = -33.3kJ -7.218kJ
Delta G = -40.518
Is this Correct?